A トリス (diisocyanide) クロミウム (chromium) 複合物は,Fe (2,2'-Bipyridine) の発光アナログである
Laura A Büldt1, Xingwei Guo1, Raphael Vogel1
1Department of Chemistry, University of Basel , St. Johanns-Ring 19 and Spitalstrasse 51, 4056 Basel, Switzerland.
Journal of the American Chemical Society
|January 6, 2017
まとめ
新しいクロム複合体とケラティングリガンドは,発光性と顕著な安定性を示し,太陽電池と照明アプリケーションにおける貴金属に代わる地球に豊富な可能性を提供します.
科学分野:
- 有機金属化学
- 材料科学
- 写真化学
背景:
- 鉄 (II) 複合体は染料感受性太陽電池の土壌に豊富な感受性物質ですが,その興奮状態の寿命は限られています.
- 貴金属はしばしば発光装置や太陽電池に用いられ 地球に豊富にある代替品の研究に 駆り立てられています
- クロミウムのような過渡金属の低酸化状態を安定させることは困難ですが,ユニークな電子特性を提供します.
研究 の 目的:
- ビデント酸ケラティングイソシアニドリガンドによる新しいクロム ((0) コンプレックスを合成し,特徴づけること.
- 新しい複合体の光物理的特性,安定性,光還元能力を調査する.
- 技術の応用における貴金属の代替品として この地球に豊富な複合物の可能性を 探求する.
主な方法:
- メタテルフェニル骨組みを備えたバイデントケラティングリガンド (CNtBuAr3NC) の合成
- ホモレプスクロム ((0) コンプレックス,Cr ((CNtBuAr3NC) の形成.
- 発光寿命測定とトリプレット・トリプレット・アニヒレーション・アップコンバージョンの研究を含む光物理的特徴付け.
- 興奮状態の酸化力を決定する電気化学分析.
主要な成果:
- 合成されたCr{CNtBuAr3NC) 3複合体は,室温で安定して発光する.
- この複合体は,アイソエレクトロニック鉄複合体を上回る非常に長い興奮状態の寿命 (2.2ns) を表している.
- Cr(CNtBuAr3NC) 3は,他のCr(0) コンプレックスと比較して,光分解に対する強化された強度を示しています.
- 効率的なエネルギー伝達とトリプレット・トリプレット・アニヒレーション・アップコンバーションがアントラゼンで観察されました.
- 複合体は, -2. 43V対Fc+/ Fcの興奮状態酸化ポテンシャルを持つ強力な光還元剤として作用する.
結論:
- 新型バイデントケラティングリガンドは,クロミウムをゼロバルント状態で効果的に安定させる.
- Cr ((CNtBuAr3NC) 3は,発光装置および染料感受性太陽電池のアプリケーションに有望な性質を示しています.
- この研究は,貴金属の持続可能な代替品として,地球に豊富なクロム複合体の可能性を強調しています.
関連する概念動画
Colors and Magnetism
14.4K
Color in Coordination Complexes
When atoms or molecules absorb light at the proper frequency, their electrons are excited to higher-energy orbitals. For many main group atoms and molecules, the absorbed photons are in the ultraviolet range of the electromagnetic spectrum, which cannot be detected by the human eye. For coordination compounds, the energy difference between the d orbitals often allows photons in the visible range to be absorbed and emitted, which is seen as colors by the human...
When atoms or molecules absorb light at the proper frequency, their electrons are excited to higher-energy orbitals. For many main group atoms and molecules, the absorbed photons are in the ultraviolet range of the electromagnetic spectrum, which cannot be detected by the human eye. For coordination compounds, the energy difference between the d orbitals often allows photons in the visible range to be absorbed and emitted, which is seen as colors by the human...
14.4K
Valence Bond Theory
11.5K
Coordination compounds and complexes exhibit different colors, geometries, and magnetic behavior, depending on the metal atom/ion and ligands from which they are composed. In an attempt to explain the bonding and structure of coordination complexes, Linus Pauling proposed the valence bond theory, or VBT, using the concepts of hybridization and the overlapping of the atomic orbitals. According to VBT, the central metal atom or ion (Lewis acid) hybridizes to provide empty orbitals of suitable...
11.5K
Formation of Complex Ions
26.5K
A type of Lewis acid-base chemistry involves the formation of a complex ion (or a coordination complex) comprising a central atom, typically a transition metal cation, surrounded by ions or molecules called ligands. These ligands can be neutral molecules like H2O or NH3, or ions such as CN− or OH−. Often, the ligands act as Lewis bases, donating a pair of electrons to the central atom. These types of Lewis acid-base reactions are examples of a broad subdiscipline called coordination...
26.5K
Crystal Field Theory - Tetrahedral and Square Planar Complexes
49.3K
Tetrahedral Complexes
Crystal field theory (CFT) is applicable to molecules in geometries other than octahedral. In octahedral complexes, the lobes of the dx2−y2 and dz2 orbitals point directly at the ligands. For tetrahedral complexes, the d orbitals remain in place, but with only four ligands located between the axes. None of the orbitals points directly at the tetrahedral ligands. However, the dx2−y2 and dz2 orbitals (along the Cartesian axes) overlap with the ligands less than the dxy,...
Crystal field theory (CFT) is applicable to molecules in geometries other than octahedral. In octahedral complexes, the lobes of the dx2−y2 and dz2 orbitals point directly at the ligands. For tetrahedral complexes, the d orbitals remain in place, but with only four ligands located between the axes. None of the orbitals points directly at the tetrahedral ligands. However, the dx2−y2 and dz2 orbitals (along the Cartesian axes) overlap with the ligands less than the dxy,...
49.3K
Structural Isomerism
22.3K
Isomerism in Complexes
Isomers are different chemical species that have the same chemical formula. Structural isomerism of coordination compounds can be divided into two subcategories, the linkage isomers and coordination-sphere isomers.
Linkage isomers occur when the coordination compound contains a ligand that can bind to the transition metal center through two different atoms. For example, the CN− ligand can bind through the carbon atom or through the nitrogen atom. Similarly, SCN− can...
Isomers are different chemical species that have the same chemical formula. Structural isomerism of coordination compounds can be divided into two subcategories, the linkage isomers and coordination-sphere isomers.
Linkage isomers occur when the coordination compound contains a ligand that can bind to the transition metal center through two different atoms. For example, the CN− ligand can bind through the carbon atom or through the nitrogen atom. Similarly, SCN− can...
22.3K
Metal-Ligand Bonds
25.2K
The hemoglobin in the blood, the chlorophyll in green plants, vitamin B-12, and the catalyst used in the manufacture of polyethylene all contain coordination compounds. Ions of the metals, especially the transition metals, are likely to form complexes.
In these complexes, transition metals form coordinate covalent bonds, a kind of Lewis acid-base interaction in which both of the electrons in the bond are contributed by a donor (Lewis base) to an electron acceptor (Lewis acid). The Lewis acid in...
In these complexes, transition metals form coordinate covalent bonds, a kind of Lewis acid-base interaction in which both of the electrons in the bond are contributed by a donor (Lewis base) to an electron acceptor (Lewis acid). The Lewis acid in...
25.2K


